A chemical engineer calculated that 15.0 mol H2 was needed to react with excess N2 to prepare 10.0 mol NH3. But the actual yield is 60.0%. Write a balanced chemical equation for the reaction. Is the amount of H2 needed to make 10.0 mol NH3 greater than, equal to, or less than 15 mol? How many moles of H2 are needed?

Question

Chemistry

Jamari Ortega

30 May, 00:14

A chemical engineer calculated that 15.0 mol H2 was needed to react with excess N2 to prepare 10.0 mol NH3. But the actual yield is 60.0%. Write a balanced chemical equation for the reaction. Is the amount of H2 needed to make 10.0 mol NH3 greater than, equal to, or less than 15 mol? How many moles of H2 are needed?

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Answers (1)

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Gilbert Gordon · Answer 1

The actual number of moles is 9 moles.

It is less than 15

Number of moles needed is 9 moles

Explanation:

15H2 + 10N2 - --> 10NH3

Now from the question, we can see that the percentage yield is 60%

The percentage yield can be calculated as actual moles of H2/Theoretical moles of H2 * 100%

From the equation, we can see that the theoretical number of moles of hydrogen is 15.

Now to get the actual : 60 = x/15 * 100

x = 9

The actual number of moles is 9 moles.

It is less than 15

Number of moles needed is 9 moles